For a first order reaction, the half-life is text10 textmins text. How much time in minutes will it take to reduce the concentration of reactant to 25 % of its original concentration?

Question

For a first order reaction, the half-life is text10 textmins text. How much time in minutes will it take to reduce the concentration of reactant to 25 % of its original concentration? (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

It takes two half-lives to reduce the concentration of reactant to 25 % of its original concentration. <img class="img-fluid question-image" alt="Solution" src="https://cdn.tardigrade.in/q/nta/c-su3g47uwb4ccqjix.jpg" /> Hence, total time taken =10+10 =20 minutes.

Q. For a first order reaction, the half-life is $10 mins .$ How much time in minutes will it take to reduce the concentration of reactant to $25%$ of its original concentration?

It takes two half-lives to reduce the concentration of reactant to $25%$ of its original concentration.
Hence, total time taken $= 10 + 10$
$= 20$ minutes.

Q. For a first order reaction, the half-life is 10mins. How much time in minutes will it take to reduce the concentration of reactant to 25% of its original concentration?

It takes two half-lives to reduce the concentration of reactant to 25% of its original concentration. Hence, total time taken =10+10 =20 minutes.

Q. For a first order reaction, the half-life is $10 mins .$ How much time in minutes will it take to reduce the concentration of reactant to $25%$ of its original concentration?

It takes two half-lives to reduce the concentration of reactant to $25%$ of its original concentration.
Hence, total time taken $= 10 + 10$
$= 20$ minutes.